MHT CET · Chemistry · Electrochemistry
Calculate \(\mathrm{E}_{\text {cell }}^{\circ}\) for the following.
\(\mathrm{Zn}_{(\mathrm{s})}\left|\mathrm{Zn}_{(1 \mathrm{M})}^{++}\right|\left|\mathrm{Pb}_{(1 \mathrm{M})}^{++}\right| \mathrm{Pb}_{(\mathrm{s})}\) if \(\mathrm{E}_{\mathrm{Zn}^{\circ}}^{\circ}=-0.763 \mathrm{~V}\) and
\(\mathrm{E}_{\mathrm{Pb}}^{\mathrm{o}}=-0.126 \mathrm{~V}\)
- A \(0.637 \mathrm{~V}\)
- B \(-0.530 \mathrm{~V}\)
- C \(-0.889 \mathrm{~V}\)
- D \(0.789 \mathrm{~V}\)
Answer & Solution
Correct Answer
(A) \(0.637 \mathrm{~V}\)
Step-by-step Solution
Detailed explanation
For the given cell, \(\mathrm{Zn}\) acts as anode and \(\mathrm{Pb}\) acts as cathode.
\(\mathrm{E}_{\text {cell }}^0=\mathrm{E}_{\text {cathode }}^0-\mathrm{E}_{\text {anode }}^0\)
\(=\mathrm{E}_{\mathrm{Pb}}^0-\mathrm{E}_{\mathrm{Zn}}^0=-0.126 \mathrm{~V}-(-0.763) \mathrm{V}\)
\(=0.637 \mathrm{~V}\)
\(\mathrm{E}_{\text {cell }}^0=\mathrm{E}_{\text {cathode }}^0-\mathrm{E}_{\text {anode }}^0\)
\(=\mathrm{E}_{\mathrm{Pb}}^0-\mathrm{E}_{\mathrm{Zn}}^0=-0.126 \mathrm{~V}-(-0.763) \mathrm{V}\)
\(=0.637 \mathrm{~V}\)
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